{"id":6008,"date":"2020-10-13T12:38:40","date_gmt":"2020-10-13T07:08:40","guid":{"rendered":"http:\/\/astan.lk\/al_virtualclassroom\/?p=6008"},"modified":"2020-10-13T12:38:42","modified_gmt":"2020-10-13T07:08:42","slug":"benzene","status":"publish","type":"post","link":"https:\/\/astan.lk\/al_virtualclassroom\/benzene\/","title":{"rendered":"Benzene"},"content":{"rendered":"<p>\u2022 Under normal conditions benzene does not answer the tests for unsaturation. Therefore, benzene cannot have a structure similar to that of a simple alkene or an alkyne.<\/p>\n<p>\u2022 Although the structure proposed for benzene by Kekule shows three double and three single bonds for the molecule, the bond length between any two adjacent carbon atoms in benzene is the same.<\/p>\n<p>\u2022 The carbon &#8211; carbon bond length of benzene is 1.39 x 10<sup>-10<\/sup> m which is in between the length of carbon \u00a0&#8211; carbon double bond (1.34 x 10<sup>-10<\/sup> m) and the length of carbon &#8211; carbon single bond (1.54 x 10<sup>-10<\/sup> m).<\/p>\n<p>\u2022 Therefore, the structure of benzene is considered to be a hybrid of the resonance structures given below.<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"\" src=\"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/7\/79\/Benz3.svg\/350px-Benz3.svg.png\" width=\"297\" height=\"158\" \/><\/p>\n<p>&nbsp;<\/p>\n<p>\u2022 The structure of benzene can be explained by molecular orbital theory. All its C atoms have undergone sp<sup>2<\/sup> hybridization. Each carbon bears an unhybridized p orbital which can overlap with the unhybridized p orbitals on either sides of it.<\/p>\n<p>\u2022 From this, a cyclic delocalized electron cloud is formed.<\/p>\n<p>\u2022 Hence, the real structure of benzene is considered to be a hybrid of two Kekule structures.<\/p>\n<p>\u2022 The real structure of benzene with delocalized electrons is more stable than the Kekule structure with three double bonds.<\/p>\n<p>\u2022 The data for the standard enthalpy of hydrogenation helps to illustrate the stability of a benzene molecule.<\/p>\n<p><img decoding=\"async\" src=\"http:\/\/www.chemguide.co.uk\/basicorg\/bonding\/hydrogeq1.GIF\" \/>\u00a0\u00a0The enthalpy change during this reaction is -120 kJ mol<sup>-1<\/sup><\/p>\n<p><img decoding=\"async\" src=\"http:\/\/www.chemguide.co.uk\/basicorg\/bonding\/hydrogeq3.GIF\" \/>\u00a0\u00a0The enthalpy change during this reaction is -208 kJ mol<sup>-1<\/sup><\/p>\n<p>But if benzene possesses three double bonds, its standard enthalpy of hydrogenation should be 3 x (-120 kJ mol<sup>-1<\/sup><br \/>\n), that is -360 kJ mol<sup>-1<\/sup><br \/>\n. Hence, benzene is more stable than its Kekule structures by an amount equal to (360-208) = 152 kJ mol<sup>-1<\/sup><\/p>\n<p>&nbsp;<\/p>\n<p><img decoding=\"async\" src=\"http:\/\/www.chemguide.co.uk\/basicorg\/bonding\/energetics.GIF\" \/><\/p>\n","protected":false},"excerpt":{"rendered":"<p>\u2022 Under normal conditions benzene does not answer the tests for unsaturation. Therefore, benzene cannot have a structure similar to that of a simple alkene or an alkyne. \u2022 Although the structure proposed for benzene by Kekule shows three double and three single bonds for the molecule, the bond length between any two adjacent carbon [&hellip;]<\/p>\n","protected":false},"author":842,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"_monsterinsights_skip_tracking":false,"_monsterinsights_sitenote_active":false,"_monsterinsights_sitenote_note":"","_monsterinsights_sitenote_category":0,"footnotes":""},"categories":[14,1666],"tags":[],"class_list":["post-6008","post","type-post","status-publish","format-standard","hentry","category-chemistry","category-unit-08"],"acf":[],"yoast_head":"<!-- This site is optimized with the Yoast SEO plugin v26.9 - https:\/\/yoast.com\/product\/yoast-seo-wordpress\/ -->\n<title>Benzene - Learning &amp; Education Portal<\/title>\n<meta name=\"robots\" content=\"index, follow, max-snippet:-1, max-image-preview:large, max-video-preview:-1\" \/>\n<link rel=\"canonical\" href=\"https:\/\/astan.lk\/al_virtualclassroom\/benzene\/\" \/>\n<meta property=\"og:locale\" content=\"en_US\" \/>\n<meta property=\"og:type\" content=\"article\" \/>\n<meta property=\"og:title\" content=\"Benzene - Learning &amp; Education Portal\" \/>\n<meta property=\"og:description\" content=\"\u2022 Under normal conditions benzene does not answer the tests for unsaturation. 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